12.57 Pheromones are compounds secreted by the females of many insect species to attract males. One of these compounds contains 80.78 percent C, 13.56 percent H,and 5.66 percent O. A solution of 1.00 g of this pheromone in 8.50 g of benzene freezes at 3.37°C. What are the molecular formula and molar mass of the compound? (The normal freezing point of pure benzene is 5.50°C.)

Can you expand the process on how to solve with the formula? In(At/A0)=-kt

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Consider The Following Reaction M Inbox (208) - eleganceextreme1 X + 05657571&snapshotld=13245488id-563649000&takeld-4bfba59b09f0e5b& X X QSearch this course X References Use the References to access important values if d for this question. *** The equilibrium constant, K,, for the following reaction is 8.46x10 at 298 K: 1 00 NH3(g) + H2Se(g) NH4HSe(s) A-Z Calculate the partial pressure of each gas and the total pressure at equilibrium when 0.469 moles of NHHSe(s) is introduced into a 1.00 L vessel at 298 K. Assume that the volume occupied by the solid is negligible. PNH3 atm atm PH2SE atm Ptotal 6. Equilibrium Calculations with Partial Pressur... : This is group attempt 1 of 5 Next Autosaved at 1:06 PM Back 1:06 PM xa 11 9/24/2019 1 hp delete rt co

Calculate the solubility of CaF2 (aq) in a solution, that is 0.015 molar in MgSO4 (aq). Compare your result to the one you obtain by using concentration instead of activities. Take the solubility product as 3.9 × 10 ^-11

Equilibrium Constant, K Test tube 1 = 75.0 Test tube 2 = 88.2 Test tube 3 = 167 Test tube 4 = 161 Test tube 5 = -49.6  For which test tube should your value for the equilibrium constant be most reliable? Justify your selection based on your data and your laboratory experience in completing this procedure.

[Rev Topics] [References] Use the References to access important values if needed for this question. Consider the following reaction where Ke = 6.30 at 723 K. 2NH3 (9) N₂(g) + 3H₂(g) A reaction mixture was found to contain 0.000687 moles of NH3(g), 0.0258 moles of N₂ (g), and 0.0435 moles of H₂(g), in a 1.00 liter container. Calculate Qc. Qc = 1 Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction must run in the forward direction to reach equilibrium. The reaction must run in the reverse direction to reach equilibrium. The reaction is at equilibrium. Submit Answer Retry Entire Group 9 more group attempts remaining Previous Next> ad Exit ? or n er

emplain the last part of the equation. how is the operation performed to achieve 84 ??